Exploring Copper's Thermal Conductivity

Copper is a transitional metal with an atomic number of 29. Its atomic mass is 63.546. A pure metal found in nature, its compounds are usually found as copper(II) salts. Copper is typically a reddish-brown with a shine or glow to it. When it is exposed to air it darkens to a brown color. If exposed to air and water, it becomes a blue-green. Its phase of matter is solid, with a melting and boiling point of 1084.62 °C and 2562 °C respectively. Copper is soft and malleable, meaning that it is capable of being pulled or stretched. Its density at room temperature is 8.96 g/cm3, and 8.02 g/cm3 when melted. Copper is characterized by its very high thermal and electrical conductivity. It is adaptable and durable. Copper does not react with water, and
These natural isotopes are 63Cu and 65Cu. 63Cu and 65Cu are stable as well. 63Cu has 29 protons, 34 neutrons, and 29 electrons. 65Cu has 29 protons and 29 electrons as well, but 36 neutrons as opposed to 34. The other isotopes are radioactive, the most stable being 67Cu.
The softness of copper partially explains its high electrical conductivity, as well as its thermal conductivity. The resistivity to electron transport in metals originates, for the most part, from the scattering of electrons on thermal vibrations of the lattice of the crystal structure, which are relatively weak for a soft metal. Prolonged defects to the crystal lattice, like grain boundaries, obstructs flow of the matter under applied stress, increasing its hardness.[7]
The reddish-brownish color of copper results from the electronic transitions between the filled 3d and half-empty 4s atomic shells; the difference of energy between the shells corresponds to orange light. Copper is located in period 4, group 11, with one s-orbital electron on top of a filled d-electron shell. The filled d-shells in these elements do not influence the interatomic interactions that much, which are controlled by the s-electrons through metallic bonds. Since copper does not have complete d-shells, the metallic bonds are lacking a covalent nature and are comparably weak. This explains the low hardness and high ductility of single crystals of
Architectural structures built with copper corrode to give green verdigris (or patina). It can often be seen on old copper constructions. Copper reacts with carbon dioxide and water to form the greenish substance. Other times, copper tarnishes when exposed to sulfides, which react with it to form various copper sulfides. It reacts with sulfurous acid rain, forming a layer of patina that is primarily made of sulfide or sulfate compounds.[11][12][13] The natural green film has been utilized by architects and designers. The tarnish that forms is very durable, and is extremely resistant to corrosion. It protects the copper underneath from further